WS16 - Chem 1319 Midterm Review Questions
1 . (MSDS) Safety and General Information:
a. What is proper attire to wear in the lab?
(goggles, long pants, closed toe shoes, when necessary gloves, aprons, labcoats)
b. In case you spill 3M HCl, what will the TA use to neutralize the spill?
(NaHCO3 otherwise known as baking soda or sodium bicarbonate.)
c. If you break an empty beaker in the lab, what should you do?
(Notify your TA to clean up the broken glass.)
d. What is the most important reason that you not eat or drink in the lab?
(So your food/drink does not become contaminated and harm you.)
e. Why is it important that separate waste containers are used for each experiment?
(So the chemicals do not react in the waste containers.)
f. Give examples of qualitative vs. quantitative observations.
(Quantitative observations involve numbers / qualitative do not.
So…
Quantitative – The worm was 4.5 cm long.
Qualitative – The worm was pink in color.)
g. What is the difference between a homogeneous and a heterogeneous mixture?
Give an example of each.
Homogeneous mixtures are uniform throughout. Heterogeneous are not.
Homogeneous = Grape Juice
Heterogeneous = Chocolate Chip Cookies.
h. What are some physical properties of oxygen? What are some chemical properties?
Physical: Oxygen is a gas at 23 oC.
Chemical: Oxygen and hydrogen react to form water.
i. What are some indications that a chemical reaction has occurred?
(Bubbles indicate evolution of a gas.
Temperature change. Exothermic = hotter. Endothermic = cooler.
Color change.
Precipitate forms.)
j. What is the main hazard of a reaction where hydrogen gas is produced?
(Hydrogen is flammable in small quantities; explosive in large ones.)
k. Why did we not use HF to dissolve the SiO2 in the ternary mixture experiment?
HF might be a weak acid, but it is more dangerous than HCl.
HF can penetrate the skin and deplete the calcium from the bones
resulting in death if not treated.
Please diregard this question as it refers to an experiment we have not done yet.
2. (D.A. #1-3) Unit conversions:
a. (1) We have a measured mass of mercury (2.00g) and a density of mercury
(13.6g/ml). Solve for the volume in liters. (0.000147 L or 1.47 x 10-4 L)
b. (1) How many weeks did it take you to read Lord of the Rings, if it took you 302,400
seconds to read it. (0.5 weeks)
c. (2) Find the number of moles of 100.0 grams of Cu(NO3)2. (0.5332 moles)
d. (2) Find the mass of 1.25 moles of C4H10. (72.655 g)
e. (3) Determine the percent composition of C4H10. (%C = 82.7% and %H = 17.3%)
3. (S.F) Scientific (a.k.a. Exponential) Notation and Significant Figures:
a. Convert to scientific notation 0.08206 (8.206 x 10-2)
b. What is the numerical value of 3.000 x 101 ? (30.00)
c. How many significant figures are there in the number 0.030100 ? (0.030100 →5)
d. Write 0.0654234 to 3significant figures. (0.0654 or 6.54x 10-2)
e. Using the correct number of significant figures, what is the answer to
3.67 kg + 12.498 kg? (Add/Subtract go with the least precise value.
In this case, is it is the hundredths place, so 16.17)
f. Using the correct number of significant figures, what is the answer when 5.18 is
multiplied by 4.2 ? (Multiply/Divide go with the least number of sigfigs.
In this case, it is two, so 22.)
4. (Zinc) Pennies that have been made after 1982 are a composite of zinc and copper. The copper is plated on top of the zinc. The zinc can be removed from the penny by cutting the coin and creating a reaction between the zinc and concentrated hydrochloric acid. The copper does not react with hydrochloric acid.
The penny was measured using Vernier calipers. The diameter was 1.79 cm and the height was 0.13 cm. The penny was weighed and the mass determined to be 2.518 grams. The penny was cut and placed in excess hydrochloric acid. After the solution stopped bubbling, the penny shell was removed. The penny shell was weighed and the mass of copper was determined to be 0.071 grams. The density of copper is 8.94 g/cm3.
a. What is the volume of copper (the copper penny shell) in the penny?
(d = m / v so v = m / d = 0.071g / (8.94 g / cm3 = 0.0079 cm3)
b. Calculate the surface area of the copper. The surface area of the copper is equal to the
surface area of the penny. The surface area of a penny can be approximated by using the
equation for the surface area of a cylinder: SAcylinder = 2(πr2) + 2πrh.
(r = 0.895 cm, so SA = 5.76 cm2)
c. Determine the thickness of the copper coating present in the penny. (T = V / SA = 0.0014 cm)
d. What is the mass percent of copper in the penny? ( (0.071g / 2.518g)x100 = 2.8%)
e. Since 1982, pennies are composed of 97.5% zinc and 2.5% copper by mass. Calculate the
percent error between the mass percent of copper in the previous answer and the
expected value. (%E = [(2.5g – 2.8g) / 2.5g] x 100 = 12%)
5. (Zinc) For the following data set (6.1, 7.2, 6.5, 4.9, 5.3, 5.9)
a. Determine the mean (average). (xAVG = 5.98, but 2 sigfigs so xAVG = 6.0)
b. Determine the standard deviation estimate. (Why are we using the standard deviation estimate and not the standard deviation?) (s. dev. est. = 0.83, because we have a small dataset.)
c. Determine the confidence interval for a single value at 90% and the confidence interval for the mean at 90% where t = 2.015. (CIsing = 1.67 or 1.7; CImean = 0.68 or 0.7)
d. How many degrees of freedom does this data set have? How do you determine degrees of freedom? (5, it is the number of trials/values minus one, so 6 – 1 = 5)
6. (E.F.) A student analyzes a sample of a material that is known to contain no elements other than molybdenum (Mo) and sulfur (S). In the student’s experiment, the mass of a sample of molybdenum sulfide, MoxSy, is determined to be 0.583 g. The sample is heated in an acid solution and H2S gas is liberated leaving only molybdenum. The final weight is 0.255 g.
a. Determine the mass percent of Mo in the sample of molybdenum sulfide, MoxSy. (43.7%)
b. Determine the mass of the S in the sample of molybdenum sulfide, MoxSy. (0.328 g)
c. Determine the mass percent of S in the sample of molybdenum sulfide, MoxSy. (56.3%)
d. Determine the empirical formula of the molybdenum sulfide sample based on the values
closest to the values calculated in a & b. The Empirical Formula for this compound is:
Mo2S3, MoS, MoS3, or MoS4(MoS4)
7. (13 TT) Balance and complete the overall reactions, then give the net ionic reactions for each of the following reactions:
All we are really doing is swapping the cations & making sure charges match and all atoms are accounted for on both sides of the arrow. It’s analogous to balancing an algebraic equation, where the arrow would be the equal sign.
a. H2SO4(aq) + Ba(NO3)2(aq) →BaSO4(s) + 2 HNO3 (aq) overall
SO42-(aq) + Ba2+(aq) → BaSO4(s)net ionic
b. 2NH4OH (aq) + Cu(NO3)2(aq) → Cu(OH)2(s) + 2 NH4NO3 (aq) overall
2 OH-(aq) + Cu2+(aq) → Cu(OH)2(s)net ionic
c. K2CrO4(aq) + Ba(NO3)2(aq) →BaCrO4(s) + 2 KNO3 (aq) overall
CrO42-(aq) + Ba2+(aq) → BaCrO4(s)net ionic
d. Fe(NO3)3(aq) + 3KSCN (aq) →Fe(SCN)3(s) + 3KNO3 (aq) overall
Fe3+(aq) + 3SCN-(aq) → Fe(SCN)3 (s)net ionic
e. Na2S (aq) + SnCl2(aq) → SnS(s) + 2 NaCl(aq) overall
S 2-(aq)+ Sn 2+(aq) → SnS(s)net ionic
f. K2C2O4 (aq) + Ba(NO3)2(aq) →BaC2O4(s) + 2 KNO3 (aq) overall
C2O42-(aq) + Ba2+(aq) → BaC2O4(s)net ionic
g. H2SO4(aq) + Na2S (aq) → H2S(g) + 2 Na SO4 (aq) overall
2 H+(aq) + S 2-(aq) → H2S(g)net ionic
8. Graphing
a. For what type of data would one use a pie chart? a bar graph? a line graph? a scatterplot? (Pie Chart for Percentages.
Bar Graph when at least one of the variables is not numeric.
Line Graph for numerical data points, where varying the dependent value, x,
affect the outcome of the independent value, y.
Scatterplot for numerical data points, where it is unclear prior to plotting
if there is a trend.
b. What do error bars indicate? When are they used?
(Standard deviation or standard deviation estimate. They are used to
indicate that the average is not exact, but falls within a range.)
9. Nomenclature
a. Name the following compounds:
NH4OHammonium hydroxideBa(NO3)2barium nitrate
CuCl2,copper (II) chloride CuNO3copper (I) nitrate
or cupric chlorideor cuprous nitrate
Fe(NO3)3iron (III) nitrate or ferric nitrateNiSO4nickel sulfate
Na2CrO4sodium chromateNa2S sodium sulfide
K2CrO4potassium chromateK2C2O4potassium oxalate
KSCNpotassium thiocyanateH2SO4sulfuric acid
SnI2tin (II) iodide Pb(CH3CO2)2lead (II) acetate
or stannous iodideor plumbous acetate
Li2CO3lithium carbonate
10. Oxidation / Reduction –We’re going to move this to the final exam.
a. Define oxidation and reduction.
Oxidation – the loss of electrons. Reduction – the gain of electrons
b. Work through the oxidation / reduction problems.
11. Molecular Modeling & Lewis Dot
a. Determine the electon configuration & lewis dot form for the following elements:
K, Mg, N, S, F
electron configuration:
K1s22s22p63s23p64s1[Ar] 4s1
Mg1s22s22p63s2[Ne] 3s2
N1s22s22p3[He]2s22p3
S1s22s22p63s23p4[Ne] 3s23p4
F1s22s22p5[He] 2s22p5
Lewis Dot:
b. Determine the electon configuration & lewis dot form for the following ions:
K+, Mg2+, N3-, S2-, F-
electron configuration:
K+1s22s22p63s23p6[Ar]
Mg2+1s22s22p6[Ne]
N3-1s22s22p6[Ne]
S2-1s22s22p63s23p6[Ar]
F-1s22s22p6[Ne]
Lewis Dot:
[K]+ / [Mg]2+ / [N]3- / [S]2- / [F]-May also be shown with 8 dots around the elemental symbol.
c. Determine the hybridization, molecular and electron geometry for the following compounds:
/ sp3 / tetrahedral / tetrahedral/ sp3d2 / octahedral / square
pyramidal
/ sp3 / tetrahedral / bent
/ sp3 / tetrahedral / trigonal
pyramidal
1